MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Henderson Hassleback Equation

In a basic bu...

Question

In a basic buffer, $0.0025$ mole of $N H_{4} C l$ and $0.15 m o l e$ of $N H_{4} O H$ are present. The $p H$ of the solution will be:
$(p K_{a}) = 4.74$

A

11.04

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

B

10.24

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C

6.62

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

5.48

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $11.04$
From Henderson's equation,

$p O H = p K_{b} + l o g \frac{[s a l t]}{[b a s e]}$

$= 4.74 + l o g \frac{0.0025}{0.15}$

$= 4.74 + l o g \frac{1}{60}$
$= 2.96$

$p H = 14 - 2.96$
$= 11.04$

Suggest Corrections

thumbs-up

0

Similar questions

Q. 1 lit of a buffer solution contains 0.1 mole each of

N H_{4} O H

N H_{4} C l

. What will be the

p^{H}

of the solution when 0.01 mole of HCl is added to it?

[P^{K b} o f N H_{4} O H = 4.74]

Q. Calculate the pH of the buffer solution containing

0.15 m o l e

{N H}_{4} O H

0.25 m o l e

{N H}_{4} C l

K_{b}

{N H}_{4} O H

1.8 \times 10^{- 5}

Q. In what volume ratio NH4Cl and NH4OH having 1M concentration should be mixed to get a buffer solution of pH=9.26 (pK_b of NH4OH = 4.74?

p K_{b}

N H_{4} O H

at certain temperature is 4.74 The pH of basic buffer containing equimolar concentration of

N H_{4} O H

N H_{C} I

Q. Which of the following represents a correct relation for a basic buffer formed by

N H_{4} O H

N H_{4} C l

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Buffer Solutions

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Henderson Hassleback Equation

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon